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The equilibrium constant, K, for the following reaction is 1.29E-2 at 600 K. COCl2(g) <--> CO(g)...

The equilibrium constant, K, for the following reaction is 1.29E-2 at 600 K.

COCl2(g) <--> CO(g) + Cl2(g)

An equilibrium mixture of the three gases in a 1.00 L flask at 600 K contains 0.297 M COCl2, 6.19E-2 M CO and 6.19E-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 3.13E-2 mol of CO(g) is added to the flask?

[COCl2] = M

[CO] = M

[Cl2] = M

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